Given the following information:A+B --- 2D Del...

Question

Given the following information:A+B ---> 2D Delta H= -707.5 kJ, Delta S= 338.0 J/KC ---> D Delta H= 504.0 kJ, Delta S= -244.0 J/KCalculate Delta G for the following reaction at 298K.A+B --->2C

Jules Bruno · Accepted Answer

We can use the following equation to solve for ΔG˚rxn of the first 2 reacitons:ΔG°rxn=ΔH°rxn-TΔS°rxnWe’re given the ΔH˚rxn and ΔS˚rxn of the reaction 1 (A+B → 2D) :ΔH˚rxn =  -707.5 kJΔS˚rxn = 338.0 J/K[readmore]We can easily solve for ΔG˚rxn. The given temperature is 298 K.ΔG°rxn=ΔH°rxn-TΔS°rxnΔG°rxn=(-707.5 kJ)(103 J1  kJ)-(298 K)(338.0 J K)ΔG˚rxn = -100,724.7 JWe’re given the ΔH˚rxn and ΔS˚rxn of the reaction 2 (C → D) :ΔH˚rxn =  504.0  kJΔS˚rxn = -244.0 J/KΔG°rxn=ΔH°rxn-TΔS°rxnΔG°rxn=(504.0 kJ)(103 J1  kJ)-(298 K)(-244.0 J K)ΔG˚rxn = 72712.5 JWe can use Hess’s Law to determine the Gibbs free energy change of the overall reaction from the given reactions:1. A+B → 2D                 ΔG1 = –100,724.7 J2. C → D                        ΔG2 = 72,712.5 JWe now need to find a combination of reactions that when added up, gives us the overall reaction.For (1): We can see that A and B are on the same side as the overall reaction with the same coefficient. This means we don’t need to manipulate this reaction and ΔG1.Current reaction sequence:A+B → 2D                 ΔG1 = –100,724.7 JFor (2): C is on the opposite side as that of the overall reaction with a different coefficient. To correct this, we need to reverse the reaction and multiply it by 2. Reversing a reaction changes the sign of ΔG.Current reaction sequence:A+B → 2D                                       ΔG1 = –100,724.7 J[ C → D] × 2 and reverse                 ΔG2= (72,712.5 J) × 2 × (–1)Adding the current sequence:A+B → 2D                                       ΔG1 = –100,724.7 J2D → 2C                                          ΔG2= -145,425.0 JAdding all of the reactions and ΔH together gives us:A+B → 2C                             ΔGnew = ΔG1 + ΔG2ΔGnew = (–100,724.7 J) + (-145,425.0 J)ΔGnew = -246,149.7 JConvert to kJ:( -246,149.7 J)(1 kJ103  J)= -246.15 kJThe Gibbs Free energy for the reaction A+B → 2C is -246.15 kJ

Problem: Given the following information:A+B ---> 2D Delta H= -707.5 kJ, Delta S= 338.0 J/KC ---> D Delta H= 504.0 kJ, Delta S= -244.0 J/KCalculate Delta G for the following reaction at 298K.A+B --->2C

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Problem: Given the following information:A+B ---&gt; 2D Delta H= -707.5 kJ, Delta S= 338.0 J/KC ---&gt; D Delta H= 504.0 kJ, Delta S= -244.0 J/KCalculate Delta G for the following reaction at 298K.A+B ---&gt;2C

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Problem: Given the following information:A+B ---> 2D Delta H= -707.5 kJ, Delta S= 338.0 J/KC ---> D Delta H= 504.0 kJ, Delta S= -244.0 J/KCalculate Delta G for the following reaction at 298K.A+B --->2C